Given the balanced chemical equation below, 2 NO(g) + 5 H2 (g) --> 2 NH3(g) + 2 H2O(g) 1. There are 4.00 moles of NO in a reaction vessel that has EXCESS H2. How much NH3should be produced in moles? In grams? 2. There are 4.00 moles of NO in a reaction vessel that has EXCESS H2. How much H2O should be produced in moles? In grams? 3. There are 4.00 moles of NO and 14.00 moles of H2 in a reaction vessel, how much NH3 should be produced in moles? In grams?
Given the balanced chemical equation below,
2 NO(g) + 5 H2 (g) --> 2 NH3(g) + 2 H2O(g)
1. There are 4.00 moles of NO in a reaction vessel that has EXCESS H2. How much NH3should be produced in moles? In grams?
2. There are 4.00 moles of NO in a reaction vessel that has EXCESS H2. How much H2O should be produced in moles? In grams?
3. There are 4.00 moles of NO and 14.00 moles of H2 in a reaction vessel, how much NH3 should be produced in moles? In grams?
4. For the previous reaction that began with 4.00 moles of NO and 14.00 moles of H2 in a reaction vessel, what is the limiting reactant? How many moles of the reactant in excess will be left over? How many grams of the reactant in excess will be leftover?
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