Questions 4 through 7 refer to the following experiment: 0.500 g of Ca metal is added to 50.0 mL of 1.0 M HCI. Once the reaction is complete, the temperature of the solution has risen from 25.2°C to 71.4°C. This reaction proceeds by the following chemical equation: Ca(s) + 2 H+ (aq) --> Ca²+ (aq) + H₂(g) What is the temperature change of the solution? Type your numerical answer, without units, in the space provided below. 46.2 QUESTION 5 What is the heat lost by the reaction, in units of kilojoules (kJ)? Assume that the density of the solution is 1.000 g/mL, and that the volume of the HCI does not change when the Ca metal is added. The specific heat of water is 4.184 J/(g-°C). Type your numerical answer (3 sig figs) in the space provided. Your answer should be reported in units of kJ, but DO NOT include the units in the answer you type! Remember to type the algebraic sign of your answer (+ or -), since this is important in calorimetry! 9.67 QUESTION 6 How many moles of Ca were used in this reaction? Remember, 0.500 g of Ca was added to the HCI solution. Type your numerical answer, without units in the space provided. Include 3 significant figures, and use the Blackboard format for scientific notation (2.67 x 10-5 should be typed as 2.67E-5). 0.0125 QUESTION 7 What is the heat of reaction per mole of Ca? Express your answer to 3 significant figures in units of kJ/mol. Be sure to include the algebraic sign (+ or -)!

Consider the explanation in the Introduction regarding the determination of qrxn, and answer the following questions about the reactions that you will be performing in this experiment. Part A: If the temperature of the HCl solution increases, did the solution absorb heat or release heat? A.)Absorbed heat B.)Released heat C.)Neither absorbed nor released heat Part b: Consider the explanation in the Introduction regarding the determination of qrxn, and answer the following questions about the reactions that you will be performing in this experiment. Based on your answer to question 1,   Will qsoln be a positive or negative quantity? A.)Positive B.)Negative C.)Zero    Part C Consider the explanation in the Introduction regarding the determination of qrxn, and answer the following questions about the reactions that you will be performing in this experiment. Based on your answers to questions part A and B,   If the temperature of the HCl solution increases, then did the reaction…

8.06 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.18 J/g. °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. KJ/mol 1 3 4 6. C 7 8 9. +/- х 100 LO

if 100 g of NaNO3 is dissolved in 500 g of 30.3 C water what will the final temperature of the solution be. delta H =26 kj

Consider the following reaction. X=Y If K. = 0.410 at 40. °C and K. = 0.675 at 90. °C, what is AH for the reaction? AH' = kJ/mol

Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.128 gg of Zn(s) is combined with enough HCl to make 54.4mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.3 ∘C to 23.7 ∘C.   Find ΔHrxn for this reaction as written. (Use 1.00 g/mL  for the density of the solution and 4.18 J/(g⋅∘C) as the specific heat capacity.) Express your answer in kilojoules per mole to two significant figures.

When 4 grams of a certain compound is dissolved in 61 grams of water in a calorimeter, the temperature of the calorimeter changes from 25.00ºC to 26.98 ºC. Assuming that the specific heat capacity for the resulting solution is 4.184 J/(g oC), and the heat for this solvation is found as x kJ, what is the value of x?

When 2.045 g of NH4NO3 (molar mass is 80.05 g/mL) is added to 100.0 mL of water at 25.09C, the final temperature of the water is 23.03C. What is the molar heat of solution (H) of NH4NO3 in kJ/mol?

If 100.0 g H2O at 20.1 °C is mixed with 100.0 g H2O at 98.4 °C, what is the final temperature of the solution mixture ?  Assume no heat is lost to the vessel in which the mixing takes place. Use CH2O = 1.00 cal/g×°C

When the substances in the equation below are at equilibrium at pressure Pand temperature T, how can the equilibrium be shifted to favor the products?CuO(s) + H2(g) Cu(s) + H2O(g)Change in enthalpy = –2.0 kJ.