16. How much heat is liberated at constant pressure when 97.7 g of calcium oxide reacts...
15. In a mixture of helium and chlorine, occupying a volume of 12.8 L at 605,6 mmHg and 21.6°C, it is found that the partial pressure of chlorine is 143 mmHg. What is the total mass of the sample? a. 31.6 g b. 0.4 g c. 8.37 g d. 1.28 g e. 7.09 g 16. How much heat is liberated at constant pressure when 97.7 g of calcium oxide reacts with 29.0 L of carbon dioxide gas, measured at 1.00...
Calcium oxide (lime) reacts with carbon dioxide to form calcium carbonate (chalk). CaO(s) + CO2(g) → CaCO3(s) ∆H = –178.4 kJ How many kilojoules of heat are evolved in the reaction of 0.500 kg CaO(s) (molar mass 56.08 g/mol) with an excess of carbon dioxide?
A.) When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3(s)→CaO(s)+CO2(g) What is the mass of calcium carbonate needed to produce 25.0 L of carbon dioxide at STP? B.) 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, what is the volume of carbon dioxide formed by the combustion...
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0 0 degrees * C , 60.1 kl of heat is released at constant pressure. What is AH for this reaction? (R = 0.0821L * atm / (Kmol)) 2Pb(s)+O 2 (g) 2PbO(s) ) When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0°C. 60.1 kJ of heat is released at constant pressure. What is AH°...
What volume of carbon dioxide is produced when 33.2 g of calcium carbonate reacts completely according to the following reaction at 25 °C and 1 atm? calcium carbonate (s) ->calcium oxide (s) + carbon dioxide(g) liters carbon dioxide How many grams of phosphorus (P4) are needed to completely consume 69.6 L of chlorine gas according to the following reaction at 25 °C and 1 atm? phosphorus (P4) ( s ) + chlorine ( g ) ->phosphorus trichloride ( l )...
Just need the answer to this one 1. How much heat is released at constant pressure if a 20.0-L tank containing 59.0 atm of hydrogen sulfide gas condenses at its boiling point of -60.0°C? The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at-60.00. (R A) 4.48 x 106 J B) 2.77 x 102 C) 7.81 x 101 D) 1.26 x 106 J E) 1.87×104 J 0.0821 L·atm/(K·mol))
CaCO3(s) = Cao (s)+CO2 (g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0 mol sample of CaCO3(s) is placed in a rigid 100. L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00 atm, while some CaCO3(s) remains in the vessel. a. Calculate...
A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules. Express your answer numerically in kilojoules.
A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules.
16. For the system CO + CO2(g) → CaCO(s) the equilibrium constant expression is a. [CO] b. 1/[CO] c. COCO/CaCO, d. Cacos/CaoCO 17. The value of K, for the reaction 2NOH). N204) is 1.52 at 319 K. What is the value of ko at this temperature for the reaction N04() → 2NOR ? b. 1.23 c. 5.74 x 10 d. 0.658 18. The value of Ke for the reaction C() + COX() -----2CO(g) is 1.6. What is the equilibrium concentration...