Calculating moles from a balanced equation, together with enthalpy changes
Somebody please help me figure out these problems (note: I don't want the answers, just the steps to solve them)
1.Given the following reaction:
4 KO2 + 2 H2O + 4 CO2 ==> 4 KHCO3 + 3 O2
How many moles of O2 will be produced if 2.18 moles of CO2 react completely?
2.4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g)
The enthalpy of the reaction DH = -1267 kJ. What is the enthalpy change (in kJ) when 3 grams of ammonia are burned?
3. 4 P + 5 O2 ==> P4O10
If you have 28.20 grams of P and 75.05 grams of O2, how many moles of each compound do you have present?
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