Question

In: Chemistry

1/ Determine the amount of heaat required to raise the temperature of 2500 grams of water...

1/ Determine the amount of heaat required to raise the temperature of 2500 grams of water form 35C degree to 57C degree. The specific heat of water is 4.18J/g*C.

2/A system releases 350. kilojoules of heat while 750. kilojoules of work are done on it. Determine the change in internal energy (△ E) of the system

3/ Afixed mass of gas is placed in a cylinder fitted with a movable piston. 2000.joules of heat are added to the gas, causing it to expand. The expanding gas caused the piston to rise, thus increasing the volume of the cylinder 4,5 liters. If the constant downward pressure of the piston on the gas was 3.5 atmospheres.Calculate the (△ E) of the gas.

4/ How many joules of heat are released to the surroundings when145.0 grams of aluminum react with an excess amount of iron(III) oxide according to the following reaction?

2AL + Fe2O3 ------> AL2O3 + 2Fe △Hrxn= -849KJ

5/ use the following reactions 1,2 and 3 to determine the enthalpy of reaction for:

N2O(g) + NO2(g) -----> 3NO(g) △Hrxn= ?

I/ N2(g) + O2 (g) ------> 2NO(g) △Hrxn=+180.7KJ

II/ 2NO(g) + O2(g) ------> 2NO2(g) △Hrxn=-113.1KJ

III/ 2N2O(g) ------> 2N2(g) + O2(g) △Hrxn=-163.2KJ

6/ A 75 gram piece of copper at 100C degree is placed in an insulated container that contains 225 grams of water at 35C degree. Determine the equilibrium temperature reached in the copper water system. The specific heat of copper is 0.385J/g*C and the specific heat of water is 4.18J/g*C. You may assume that there is no exchange of heat between the system and surroundings.

Solutions

Expert Solution

1) heat,q=mcT=2500 g*4.18J/g*C* (57-35)C=229900J

2)U=q + W    W=work done

         =350 kj +750 kj=1100kj

3) U=q-pV+W(non-expansion)=2000J-3.5 atm* 101325 Nm2/atm *1000m3=2000J-354.64J=1645.3J

V=5-4=1 dm3=1 (10-1)3 m3=10^-3m3

(1 atm = 101325 Pa=N/m2)

4)molar mass of Al=27g/mole

2 moles of Al=2*27g=54 g Al reacts with excess amount of iron(III) oxide to give heat=-849KJ

                               so,145 g Al reacts to give heat=-849kj/54g *145g=-2279.7kj

5) 2N2O(g) ------> 2N2(g) + O2(g)

N2O(g) ------> N2(g) + 1/2 O2(g) △Hrxn=-163.2KJ/2=-81.6kj.....(.1)

2NO(g) + O2(g) ------> 2NO2(g)

NO2(g)-----------NO(g) + 1/2 O2(g) △Hrxn=113.1KJ/2=56.55kj.......(2)

N2(g) + O2 (g) ------> 2NO(g) △Hrxn=+180.7KJ.........(3)

now eqn 1+2+3gives   N2O(g) + NO2(g) -----> 3NO(g) △Hrxn= -81.6kj+56.55kj+180.7KJ.=155.65Kj

6)q=mcT

75 g * 0.385J/g*C*(100-T)C=225 g*4.18J/g*C*(T-35)(heating)

T= equiibrium temp

100-T/T-35=32.57

100-T=32.57T-1139.95

1239.95=33.57T

T=36.9C


Related Solutions

Part B The amount of boiling water required to raise the temperature of 25.0 kgof water...
Part B The amount of boiling water required to raise the temperature of 25.0 kgof water in the bath to body temperature is 4.80 kg. In this process, the heat lost by the boiling water is equal to the heat gained by the room-temperature water. How much heat was transferred in this process? Express your answer to four significant figures and include the appropriate units. n this problem answers are requested to three significant digits for grading purposes. The true...
How many grams of steam at 100 deg.Celsius would be required to raise the temperature of...
How many grams of steam at 100 deg.Celsius would be required to raise the temperature of 43.6 g solid benzene (C6H6) from 5.5 oC to 30.0 oC? Assume that heat is only transfered from the steam (and not liquid water) and that the steam/water and benzene are seperated by a glass wall and do not mix. (The melting point of benzene is 5.5 oC; ΔHfus for benzene is 9.87 kJ/mol; specific heat for benzene is 1.63 J/g ooC; ΔHvap for...
How much energy is required to raise the temperature of 100g of water from -10 to...
How much energy is required to raise the temperature of 100g of water from -10 to 110°C?
How much heat is required to raise the temperature of 250 ML of water from 20-degree...
How much heat is required to raise the temperature of 250 ML of water from 20-degree Celcius to 35 degrees Celcius? How much heat is lost by the water as it cools back down to 20 degrees Celcius?
100 grams of boiling water (temperature 100
100 grams of boiling water (temperature 100
1. Determine the amount of heat (enthalpy) produced if 25.00 grams of hexadecane is burned in...
1. Determine the amount of heat (enthalpy) produced if 25.00 grams of hexadecane is burned in excess oxygen to produce carbon dioxide and water. Ensure that your answer includes the molecular formula and a balanced chemical equation for the combustion reaction. 2. Calculate the mass of CO2 produced from 25.00 grams of hexadecane.
When 5.00 grams of sodium hydroxide dissolves in 100. grams of water the temperature rises from...
When 5.00 grams of sodium hydroxide dissolves in 100. grams of water the temperature rises from 25.0 oC to 38.0 oC. Is this reaction endothermic or exothermic? EXPLAIN. Calculate the value of ∆H (kJ/mol) and its sign. Draw an enthalpy graph and clearly label all parts.
Natural gas (CH4) is burned to raise the temperature of 20 L of water in a...
Natural gas (CH4) is burned to raise the temperature of 20 L of water in a storage tank from 5.8 °C to 82.0 °C. a) How much heat energy (in J) is absorbed by the water? b) Assuming this was a closed system, how much heat energy (in J) was released by the burning natural gas? c) What mass (in kg) of methane was burned? d) If some heat released by the burning of natural gas was “lost” heating up...
Calculate the amount of water (in grams) that must be added to (a) 9.00 g of...
Calculate the amount of water (in grams) that must be added to (a) 9.00 g of urea [(NH2)2CO] in the preparation of a 8.10 percent by mass solution: (b) 28.9 g of MgBr2 in the preparation of a 2.90 percent mass solution:
50.0 grams of cold water is placed in a styrofoam calorimeter and the initial temperature of...
50.0 grams of cold water is placed in a styrofoam calorimeter and the initial temperature of this water is 22.0 C. then 50.0 grams of warm water, initially at 40.0 C, is added to the cold water and the final temperature of the mixture is 30.6 C. Calculate: a) heat absorbed by cold water; heat lost by warm water, anc c) heat capacity of calorimeter
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT