If I want to make 12 g of XeO2 from the elements, how much Xe do I need, in grams

a) If 42.1 mL of 1.02 M sodium hydroxide, measured using a graduated cylinder, is placed in a beaker filled with 300 mL of DI water, what is the concentration of the diluted NaOH solution?

b) Why does this calculation only provide an estimate of the NaOH concentration? In other words, why do we have to standardize the NaOH in this experiment to find its exact concentration? (Hint: think about the glassware

What is the equilibrium concentration of PO4 in a 0.511 M solution of H3PO4 (Ka1 = 7.5E-3, ka2= 6.2E-8, ka3= 4.8E-13) I troes using the 5% rule but when i checked my work i was at 11%. I dont know how to solve this if i cant use the 5% rule. Help please.

To convert from a given quantity of one reactant or product to the quantity of another reactant or product:

First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02×1023 particles per mole) to convert number of particles to moles.

Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation

2H2+O2→2H2O

the coefficients tell us that 2 mol of H2 reacts with 1 mol of O2 to produce 2 mol of H2O.

Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles.

part A. How many grams of NH3 can be produced from 3.19 mol of N2 and excess H2.

part B. How many grams of H2 are needed to produce 14.94 g of NH3?

part C. How many molecules (not moles) of NH3 are produced from 3.33×10⁻⁴ g of H2?

2. When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is

CH4(g)+O2(g)→CO2(g)+H2O(g)

This type of reaction is referred to as a complete combustion reaction.

Part a. What mass of carbon dioxide is produced from the complete combustion of 2.00×10⁻³ g of methane?

Part b. What mass of water is produced from the complete combustion of 2.00×10⁻³ g of methane?

Part c. What mass of oxygen is needed for the complete combustion of 2.00×10⁻³ g of methane?

3. Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction:

2Al(s)+3Cl2(g)→2AlCl3(s)

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction:

2Al(s)+3Cl2(g)→2AlCl3(s)

Part a. What is the maximum mass of aluminum chloride that can be formed when reacting 31.0 g of aluminum with 36.0 g of chlorine?

Express your answer to three significant figures and include the appropriate units.

4.

Determine the balanced chemical equation for this reaction.

C8H18(g)+O2(g)→CO2(g)+H2O(g)

Enter the coefficients for each compound in order, separated by commas. For example, 1,2,3,4 would indicate one mole of C8H18, two moles of O2, three moles of CO2, and four moles of H2O.

5. 1.66 g H2 is allowed to react with 10.3 g N2, producing 1.62 g NH3.

Part A

What is the theoretical yield in grams for this reaction under the given conditions?

Express your answer to three significant figures and include the appropriate units.

You are given 31.0 g of aluminum and 36.0 g of chlorine gas.

Part B

What is the percent yield for this reaction under the given conditions?

Express your answer to three significant figures and include the appropriate units.

15- Propane gas flows into a combustion chamber at a rate 250 L/min at 2.0 atmand ambient temperature. Air is added to the chamber at 1.0 atm and the same temperature. The gases are ignited.

a) To get complete combustion of the propane to carbon dioxide and water three times as much oxygen as is stoichiometrically appropriate is required. Assuming air is 21% oxygen and 79% nitrogen, calculate the required flow rate of air?

b )Under the conditions in part a, the combustion is not complete and a mixture of carbon dioxide and carbon monoxide is produced. It is determined that 94.0% of the carbon in the exhaust gas is present as carbon dioxide. The remainder is carbon monoxide. Calculate the percent composition of the exhaust gas in terms of mole fraction of CO, CO2 , O2 , N2 , and H2O. Assume the propane is completely reacted and the nitrogen is totally unreacted.

Can you please explain part B? I got 476.190 mL/min for part A.

Why is there more than one definition of acid-base behavior? Which definition is the right one?

What is the pH of the buffer that results when 0.235 mol of NH3 and (2.46x10^-1) mol of NH4Cl are dissolved in water to a volume of 0.50 L? (Ka of NH4(+) = 5.6E-10)

8.0g of aluminum at 200?C and 21g of copper are dropped into 45cm3 of ethyl alcohol at 15?C . The temperature quickly comes to 27?C.

What was the initial temperature of the copper?

Complete and balance the precipitation reactions. Include physical states in your equations. Click here for solubility rules.

A.) AgNO3(aq)+NaCl(aq)----->

B.) K3PO4(aq)+MgCl2(aq)----->

When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced. What is the empirical formula of the compound?

For each of the following pairs of aqueous solutions (all are at 300 K, unless otherwise stated), circle the one that has a higher concentration of solute:

1. 1.75 M NaCl or 1.75 m NaCl

2. 1.0% by mass KI or 1.0% by mass KBr

3. a saturated solution of n-butanol (CH3(CH2)2(CH2OH) or a saturated solution of n-decanol (CH3(CH2)8CH2OH)

4. a saturated solution of O2 at 298 K or a saturated solution of O2 at 358 K

5. a saturated solution of He under 1 atm of He or a saturated solution of Xe under 1 atm of Xe

**It would be very very helpful if you can provide an explanation for each one**

A volume of 84 mL of 0.060 M NaF is mixed with 28 mL of .15 M Sr(NO3)2. Calculate the concentrations of the following ions in the final solution (Ksp for SrF2 is 2.0x10^-10)

2C₂H_2(g) + 5O_2(g) ---> 4CO_2(g) + 2H₂O_(l)

A. Write the standard enthalpy of formation equations for those that apply:

B. Manipulate these equations and calculate the enthalpy of reaction:

C. Use the enthalpy of reaction equation and the enthalpy of formations to check your work for (B)