Given the following reactions, what is the reaction enthalpy for 3 C(graphite) + 4 H2(g) · →> C3H8(g)? C3H8(g) +2 021 → 3 C(graphite) + 4 H₂O(l) AH°=-1036 kJ/mol H2(g) + O2(g) →> H2O(l) AH°=-285 kJ/mol О A. -1321 kJ/mol B. -751 kJ/mol о C. -104 kJ/mol о D. 75 kJ/mol

Using the equations H₂ (g) + Cl₂ (g) → 2 HCI (g) AH° = -184.6 kJ/mol C (s) + 2 Cl₂ (g) →→ CCI (g) AH° = -95.7 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction C (s) + 4 HCI (g) → CCI (g) + 2 H₂ (g). 4 2

What is the standard enthalpy change for the reaction: 2C5H10(1) + 15O2(g) → 10CO2(g) + 10H20(1); where C5H10(1) AH°f = –605.0 kJ/mol; CO2(g) AH°f = -393.5 kJ/mol; H2O(1) AH°F - 285.8 kJ/mol. O a. -5583 kJ O b. -5783 kJ O C. -5383 kJ O d. -5183 kJ e. -4983 kJ

Write a balanced equation for the reaction between gaseous methane (CH4)(CH4) and fluorine gas to produce gaseous carbon tetrafluoride and gaseous hydrogen fluoride. Include phases. balanced equation:   Calculate the standard enthalpy of reaction (Δ?∘rxn).(Δ⁢Hrxn∘). Use the standard enthalpy of formation values in this table of thermodynamic properties. For carbon tetrafluoride, use Δ?∘f=−933.2 kJ/mol.Δ⁢Hf∘=−933.2 kJ/mol. Δ?∘rxn=Δ⁢Hrxn∘=   Suppose that 0.433 mol0.433 mol of methane gas is reacted with 0.904 mol0.904 mol of fluorine gas. Assuming the reaction occurs at constant pressure, how much heat is released? amount of heat released:

The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5  × 104 kJ of heat?                                            2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ

When a 45.0 g sample of an alloy at 100.0 °C is dropped into 55.0 g of water at 25.0 °C, the final temperature is 30.4 °C. What is the specific heat of the alloy? The specific heat of H2O(l) is 4.184 J·g–1·°C–1.            (A) 0.397 J·g–1·°C–1.           (B) 0.447 J·g–1·°C–1.           (C) 1.28 J·g–1·°C–1.           (D) 1.55 J·g–1·°C–1.

1/2 O2(g) + H2(g) → H2O(l)                  ΔHrxn = ?

A 0.692 g sample of glucose (C6H1206) is burned in a bomb calorimeter. The temperature of 575g of water in the calorimeter rises from 21.70 °C to 25.22 °C. If the heat capacity of the bomb is 650 J.Kl and the heat capacity of the water is 4.184 J/gK-1, calculate the heat evolved per 0.692 g of glucose.

Question 9 of 24 Determine the enthalpy of reaction for HCI(g) + NaNO2(s) → HNO2(1) + NaCI(s) 2NACI(s) + H2O(1) → 2HCI(g) + Na20(s) AH° = -507.1 kJ/mol NO(g) + NO2(g) + Na,0(s) → 2NANO2(s) AH° = -427.0 kJ/mol NO(g) + NO2(g) → N20(g) + O2(g) AH° = -43.01 kJ/mol 2HNO2(1) → N,0(g) + O2(g) + H2O(1) AH° = +34.02 kJ/mol %3D %3D %3D Tap here or pull up for additional resources @ #3 24 & 2 8.

When 0.0300L of 0.500 M KOH is mixed with 0.0500 L of 0.300 M HNO3 in a coffee-cup calorimeter, the temperature rises from 18.89°C to 20.20°C. The heat capacity of the calorimeter apparatus is 111 J/K. Calculate AH (in J) for the reaction: KOH(aq) + HNO3(aq) → KNO3(aq) + H2O(1) Assume the total volume of the solution mixture is 0.0800 L with a specific heat of 4.18 J/K•g and the density of 1.04 g/mL.