1.
m = 1.50g
c = 0.90J/g-K
T1 = 23.20C
T2 = 30.50C
q = mcT
= 1.50*0.9*(30.5-23.2)
=9.855J >>>>answer
2.
2Ba(s) + O2(g) ------------> 2BaO(s) H = -1107KJ
2 moles of Ba completely react with excess of O2 to releases energy is -1107KJ
2*137.327g of Ba completely react with excess of O2 to release energy is -1107KJ
15.75g of Ba completely react with excess of O2 to release energy = -1107*15.75/(2*137.327) = -63.5KJ >>>>answer
1. How much heat is needed to raise the temperature of 1.50 g of aluminum metal...
1. How much heat is needed to raise the temperature of 1.50 g of aluminum metal from 23.2 °C to 30.5 °C? (Specific heat capacity of aluminum is 0.90 J/g-K). 2. Given the following thermochemical equation: DH = -1107 kJ How many kJ of heat are released when 15.75 g of Ba(s) reacts completely with oxygen to form BaO(s)? 3. Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.25 g naphthalene is burned in a bomb calorimeter, the temperature rises from 25.25...
help The value of H° for the reaction below is -1107 kJ: 2Ba (s) + O2 (g) 2BaO (s) How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form BaO (s)? 23.2 kJ 26.3 kJ 96.3 kJ 46.4 kJ 193 kJ
please show me how to get the correct answers in preperation for my upcoming exam 20.) A 21.) A 20) The value of AH° for the reaction below is -1107 k]: 2Ba (s) +O2 (g)2BaO (s) How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form BaO (s)? A) 23.2 kJ D) 96.3 kJ C) 26.3 kJ E) 46.4 kJ B) 193 kJ 21) The value of AH° for the following...
The value of AH for the reaction below is -1107 kJ: 2Ba(s) + O2 (g) - 2 BaO(s) What is the value of q in kJ when 3.300 mole of Ba (s) reacts completely with oxygen to form Bao (s)? O-63.50 1827 63.50 2435 1384
QUESTION 1 According to the following thermochemical equation, what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO2. SiO2(s) + 4 HF(g) SiF4(g) + 2 H20) AH®rxn = -184 kJ 1079 150.9 173 g 37.59 QUESTION 2 The value of AH® for the reaction below is -1107 kJ: 2Ba (s) + O2(g) + 2Bao (s) How many kJ of heat are released when 5.75 g of Bao (s) is produced? 96.3...
NEED ANSWER ASAP A sample of aluminum metal absorbed 11.2 J of heat. The temperature of the sample increased from 23.2 °C to 30.5 °C. The specific heat of aluminum is 0.90 J/g °C. What is the mass of the sample in grams? 0 72 g O 1.7 g O 119 O 65 g O 7.3 g
How much heat is required to raise a 5.38 g sample of aluminum (26.98 g/mol) from 29.0°C to a temperature of 894°C? The information below may be useful. Specific heat capacity of Al (solid) = 0.903 J/g x *C Specific heat capacity of Al (liquid) = 1.18 J/g x *C ΔHfusion = 10.7 kJ/mol Melting Point of Al = 660*C
According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g/mol B2H6(g)6 Cl2(g)2 BCI3(g) +6 HCl(g) AHorxn-1396 kJ O 238 kJ O 1640 kJ O 429 kJ O 1430 kJ O 3070 kJ QUESTION 2 0.5 points Save Answer The value of AH° for the reaction below is -1107 kJ: 2Ва (s) + O2 (g) — 2ВаО (s) How many kJ of...
How much heat (in kJ) is required to raise the temperature of 288.7 g of ethanol (mw=46.07) from 39.38 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)
How much heat (in kJ) is required to raise the temperature of 202.8 g of ethanol (mw=46.07) from 40.34 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)