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Type the correct answer in each box. express your answer to two significant figures. you form water vapor by mixing oxygen and hydrogen at 730°c in a 5.4-liter container. this is the equation for the reaction: o2(g) 2h2(g) → 2h2o(g). the partial pressure of oxygen before the reaction is 122.3 kilopascals, and there is excess hydrogen. how many moles of water are formed? the reaction produces moles of water.

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The number of moles of water vapor formed in the reaction is 0.158 moles

What is the ideal gas equation?

The ideal gas equation shows the relationship between number of moles, temperature, volume and pressure.

Now;

P = 122.3 kilopascals or 1.21 atm

V = 5.4 L

T = 730°c or 1003 K

n = ?

R = 0.082 atmLK-1mol-1

PV = nRT

n = PV/RT

n =  1.21  *  5.4/0.082 * 1003

n = 6.53/82.2

n = 0.079 moles

The equation of the reaction is; O2 (g) + 2H2(g) ---->2H2O(g)

If 1 mole of O2 formed 2 moles of H2O

0.079 moles of O2 yield x moles of H2O

x = 0.079 * 2/1

= 0.158 moles

Learn more about ideal gas equation:https://brainly.com/question/4147359

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