Calculate ΔH for the reaction. Show your calculation. How many steps does this reaction appear to be? How would you explain the value of 62 kJ (i.e., what does this value represent)?

You mix 122 ml of 0.249 M LIOH with 122 ml of 0.55 M HF in a coffee-cup calorimeter, and the T of the solution rises from 21.0°C to 28°C (what does that mean T increasing?). What is the enthalpy of reaction/mole of LiF (AH in kJ/mol??)? Assume density of the solutions are all 1.00 g/ml, and the c of the solutions are 4.2 J/gK. Use the correct sign (+ vs -). Enter to 1 decimal place with the correct sign (+ or -).

1. What is 4-H for this reaction: 3C(s) + 4H2(g) → C3H8(g) given the following reactions: C3H8(g) +502(g) → 3CO2(g) + 4H2O(g) C(s) + O2(g) → CO2(g) 4-H = -2043 kJ/mol AH = -393.5 kJ/mol 4,H= -483.6 kJ/mol 2H₂(g) + O2(g) → 2H₂O(g) (a) -4191 kJ/mol (b) 1166 kJ/mol (c) 378 kJ/mol (d) -105 kJ/mol

Calculate the standard enthalpy of reaction for the combustion of methane. Round to the nearest whole number.CH4(g) + O2 --> CO2(g) + 2H2O(l) kJ/mol Compound Hf (kJ/mole) CH4(g) -75 CO2(g) -394 H2O(l) -284 This reaction is: endothermic or exothermic

Lightweight camping stoves typically use white gas, a mixture of C5 and C6 hydrocarbons. Calculate the fuel value of C5H12, given that ΔH°comb= –3535 kJ/mol. How much heat is released during the combustion of 1.30 kg of C5H12? How many grams of C5H12 must be burned to heat 1.35 kg of water from 21.0 °C to 98.1 °C? Assume that all the heat released during combustion is used to heat the water.

Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l)                     ΔH1HA(aq) → H+(aq) + A-(aq)                        ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l)        ΔH3Choose the equation that shows the correct relationship between their enthalpy changes.

9. A 40.0 kg industrial calorimeter has an overall specific heat capacity of 1.00 J/ (g°C). Complete combustion of 1.00 g of hydrogen in this calorimeter causes a temperature increase of 3.54°C. Calculate the molar enthalpy of combustion for hydrogen from this evidence. (-286 kJ/mol)

Please help me solve this question, i keep getting it wrong everytime

CHAPTER 5 - PRINCIPLES OF CHEMICAL REACTIVITY: EN Previous Page 3 of 5 endothermic ✓ exothermic When 1 mole of I2 (g) reacts with Cl₂ (g) to form ICI(g) according to the following equation, 26.8 kJ of energy are evolved. 1₂ (9) + Cl₂ (9) → 21C1(g) What is the value of q? kJ NOV 11 Next → othermic or exothermic? #tv ♫ P 100 Use the References to access DO Cengage Learning | C MacB

For the reaction below (which will be labeled reaction A), the reaction enthalpy is unknown:                                                   2 B    + 3 H2    B2H6    HA  = ? Use the following thermochemical data to calculate the reaction enthalpy ΔHA: Reaction 1:       4 B + 3 O2 → 2 B2O3                               ΔH1 = –2509 kJ Reaction 2:       2 H2 + O2 → 2 H2O                          ΔH2 = –572 kJ Reaction 3:       B2H6 + 3 O2 → B2O3 + 3 H2O   ΔH3 = –2,159 kJ Calculate the enthalpy of reaction A (in kJ) and enter the numerical value in the answer box. Do not write units in the answer box. Clearly show on a paper how each reaction can be combined to equal reaction A  (multiply or reverse  each of the above reactions).complete work must be uploaded