Answer:
approx 2.45g
Explanation:
2HCl + Na2SO4 → 2NaCl + H2SO4
2 : 1 : 2 : 1
0.05 0.025 (moles)
⇒ mH2SO4 = 0.025 × 98 = 2.45 g
Answer:
The enthalpy change of the reaction is -66.88 kJ/mol.
Explanation:
Mass of the solution = m = 100 g
Heat capacity of the solution = c = 4.18 J/g°C
Initial temperature of the solutions before mixing = 
Final temperature of the solution after mixing = 
Heat gained by the solution due to heat released by reaction between HCl and silver nitrate = Q


Heat released due to reaction = Q' =-Q = -334.4 J
Moles of silver nitrate = n
Molarity of silver nitrate solution = 0.100 M
Volume of the silver nitrate solution = 50.0 mL = 0.050 L ( 1 mL = 0.001 L)


Enthalpy change of the reaction = 

1 J = 0.001 kJ
The enthalpy change of the reaction is -66.88 kJ/mol.
3, 9, 16 are correct! 17 should be b because buffered means that it resists change in pH
Answer:
The answer to your question is P = 1.95 atm
Explanation:
Data
Pressure = P = ?
number of moles = n = 0.122
Volume = V = 1.5 l
Temperature = T = 20°C
Constant of ideal gases = 0.082 atm l/mol°K
Process
1.- Convert temperature to °K
T = 20 + 273
T = 293°K
2.- Write the formula of ideal gases
PV = nRT
-Solve for P
P = nRT/V
3.- Substitution
P = (0.122 x 0.082 x 293) / 1.5
4.- Simplification
P = 2.93 / 1.5
5.- Result
P = 1.95 atm