Question
In: Chemistry
Silicon nitride (Si3N4) is made by combining elemental silicon with nitrogen gas at a high temperature....
Silicon nitride (Si3N4) is made by combining elemental silicon with nitrogen gas at a high temperature. a.) How many grams of silicon are needed to react with an excess of nitrogen to prepare 150. grams of silicon nitride? b.) How many grams of nitrogen would need to react? c.) If you determine that 0.950 moles of silicon nitride were formed in this reaction, what would be the percent yield? Give two possible explanations for why the percent yield would be that value.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
What are silicon carbide and silicon nitride, what are their strength and hardness?
What are silicon carbide and silicon nitride, what are
their strength and hardness?
At high temperatures, coke reduces silica impurities in iron are to elemental silicon. SiO2(s) + 2...
At high temperatures, coke reduces silica impurities in iron are
to elemental silicon.
SiO2(s) + 2 C(s) arrow sign Si(s) + CO(g)
Use the table to calculate the values of AH degrees, AS degrees,
and AG degrees for this reaction at 25 degrees C.
AH
(kJ mol-1 AG (kJ
mol-1) AS (J mol-1k-1)
SiO 2(s)
-910.7
856.3
41.5
C(s)
0
0
5.7
Si(s)
0
0
18.8
Co(g)
0
-137.2
197.6
Gibbs free energy for the reaction is_____________kJ
At high temperatures, coke reduces silica impurities in iron are to elemental silicon. SiO2(s) + 2...
At high temperatures, coke reduces silica impurities in iron are
to elemental silicon.
SiO2(s) + 2 C(s) arrow sign Si(s) + CO(g)
Use the table to calculate the values of AH degrees, AS degrees,
and AG degrees for this reaction at 25 degrees C.
AH
(kJ mol-1 AG (kJ
mol-1) AS (J mol-1k-1)
SiO 2(s)
-910.7
856.3
41.5
C(s)
0
0
5.7
Si(s)
0
0
18.8
Co(g)
0
-137.2
197.6
Gibbs free energy for the reaction is_____________kJ
1. A sample of nitrogen gas at a pressure of 0.947 atm and a temperature of...
1. A sample of nitrogen gas at a pressure of 0.947 atm and a
temperature of 213 °C, occupies a volume of 687 mL. If the gas is
cooled at constant pressure until its volume is 570 mL, the
temperature of the gas sample will be 2. A helium-filled weather
balloon has a volume of 615 L at 23 °C and 754 mm Hg. It is
released and rises to an altitude of 7.93 km, where the pressure is
323...
A gas of nitrogen molecules is at a temperature of 1000K. In this case molecule has...
A gas of nitrogen molecules is at a temperature of 1000K. In
this case molecule has 3 translational, 2 rotational, and 2
vibrational degrees of freedom per molecule, i.e. a total of 7.
1.9. [1pt] Assuming the cycle operates as an engine, calculate
the engine efficiency.
ANSWER
1.10. [1pt] If you are to build the most efficient engine using
the highest and the lowest temperatures available from #9 how would
the cycle look like on a PV-diagram [you need to...
The ideal gas heat capacity of nitrogen varies with temperature. It is given by: Cp =...
The ideal gas heat capacity of nitrogen varies with temperature.
It is given by: Cp = 29.42-(2.170 *10-3) T +
(0.0582*10-5) T2 + (1.305*10-8)
T3 – (0.823*10-11) T4. T is in K
and Cp is in Joule/(mole K). Assuming that N2 is an ideal gas:
A) How much internal energy (per mole) must be added to nitrogen
to increase its temperature from 450 to 500 K.
B) Repeat part A for an initial temperature of 273 K and final
temperature...
An oxide of nitrogen was found by elemental analysis to contain 30.4% nitrogen and 69.6% oxygen....
An oxide of nitrogen was found by elemental analysis to contain
30.4% nitrogen and 69.6% oxygen. If 23.0 g of this gas were found
to occupy 5.6 L at STP, what are the empirical and molecular
formulas for this oxide of nitrogen?
Express the empirical and molecular formulas for this oxide of
nitrogen, separated by a comma.
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia....
Nitrogen and hydrogen combine at high temperature, in the
presence of a catalyst, to produce ammonia. After complete
reaction, how many molecules of ammonia are produced? How many
molecules of H2 remain? How many molecules of N2 remain? What is
the limiting reactant? Assume 4 molecules of nitrogen and 9
molecules of hydrogen are present.
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia....
Nitrogen and hydrogen combine at high temperature, in the
presence of a catalyst, to produce ammonia.
N2(g)+3H2(g)-->2NH3(g)
Assume 0.210 mol N2 and 0.664 mol H2 are present initially.
1.)After complete reaction, how many molecules of ammonia are
produced?
2.How many molecules of H2 remain?
3.How many molecules of N2 remain?
4.What is the limiting reactant, Hydrogen or Nitrogen?
nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia....
nitrogen and hydrogen combine at high temperature, in
the presence of a catalyst, to produce ammonia. N2(g)+3H2(g) >
2NH3(g). assume 0.270 mol of N2 and 0.877 mol of H2 are present
initially. Questions- 1. after complete reaction, how many moles of
ammonia are produced? 2. how many moles of H2 remain? 3. how many
moles of N2 remain? 4. what is the limiting reactant(hydrogen or
nitrogen)?
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