2y of water from 25.60°C to 34.80°C. s LThat is the heat evolvedter from 25,60°C

Question

2y of water from 25.60°C to 34.80°C. s LThat is the heat evolvedter from 25,60°C to 34.80°c. . 2.55 kJ c. 9.15 kJ C3 S. 1.35 kJ e. none of these 0.0 g sample of a metal at 100.0°C is added to 45.0 g of water at 22.00 C, the final temperature of oth the water and metal is 32.81°C. The specific heat of water is 4.184 J/gk. What is the specific heat of the bo metal? a. 33.9 JIgk b. 0.339 J/gK 505 J/gk 0.199 J/ghk e. none of these 62. When 10.0 g of ethane. C2H8(g), burns in oxygen, 519 kJ of heat are released. What is H for the thermochemical equation: 2c,He(g) + 702(g) 4C02(g) + 6H20(1) a. +3.12 x 103 kJ 10.04 :0.31 32.084 9 (tte +1.56 x 103 KJ 3.12 x 103 kJ d.-1.56 x 103 KJ e. none of these 63. Given the thermochemical equations CH4 (g) + 202(g) CO2(g) + 2H20(l)aH·890 kJ -GHa(g) + 302(g) 2CO2(g) + 2H2O(l) dH 1410 kJ) What is the H for the reaction: 2CH4 (g) + O2(g) C2H4 (g) + 2H20(1) a. 3190 kJ b. -2300 kJ C. -520 kJ d.-370 kJ e. none of these 8) 3000 3-2-5

Explanation / Answer

61.

Heat change = mass * specific heat * change in temperature

And

Total heat change = 0

45.0 * 4.184 * (32.81 - 22) + 60.0 * s * (32.81 - 100) = 0

2035.3 - 4031.4 * s = 0

s = specific heat of metal = 0.505 J.g-1.0C

(c)

63.

do 2 * (1) - 1* (2) to get the required equation.

So, deltaH = 2 (- 890 ) - 1 ( - 1410 ) = - 370 kJ

(d)

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