Number of moles of H2 = 4.85 g / 2.016 g/mol = 2.41 mole
From the balanced equation we can say that
2 mole of H2 requires 572 kJ of heat so
2.41 mole of H2 will require
= 2.41 mole of H2 *(572 kJ of heat / 2 mole of H2)
= 688 kJ of heat
Therefore, the amount of heat produced would be +688 kJ
Question 3 1 pts Given the balanced chemical equation, 2 H2O(l) - 2H2 (8) + O2(8)...
Consider the following balanced equation: 2H2 + O2 --------> 2H2O If you start with 8.133 g of H2 and 3.425 g of O2, find the following: a) With excess O2, what mass (grams) of H2O would be produced by the H2? b) With excess H2, what mass (grams) of H2O would be produced by the O2? c) What is the chemical formula for the limiting reactant?
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Question 1 2 pts Given the balanced chemical equation: Thermometer Ba(NO3)2(aq) + Na2SO4(aq) →BaSO4(s) + 2 NaNO3(aq) - Stirrer A 0.30 L of 0.15 M Ba(NO3)2(aq) is mixed with excess Na2SO4(aq) to make 200.0 g of solution in a coffee-cup calorimeter and allowed to react completely. The temperature of the solution rises from 23.5 °C to 24.9 °C. Answer the question in each step to find Hrxn for this reaction. Cs,soln = 4.18 J/g °C Cover Step 1: The reaction...
Consider the following chemical reaction. 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.3 L of O2 at a temperature of 310 K and a pressure of 0.948 atm ? Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atm and 23 ∘C, how many liters of carbon dioxide are formed by the combustion of 4.00 g of butane?
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From the following balanced equation, 2H2(g)+O2(g)⟶2H2O(g) how many molecules of H2O can be formed from 5.58mol H2?
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