Consider the following reaction: H2O(.ℓ .) arrow H2O(.g.);(ΔH)1=50kJ 2(CH)3OH(.ℓ .)+3O2(.g.) arrow 4H2O(.ℓ .)+2(CO)2(.g.);(ΔH)2=-1500kJ What is the value of ΔH for second reaction if water vapour instead of liquid water is formed as product ?

Question

Consider the following reaction: H2O(.ℓ .) arrow H2O(.g.);(ΔH)1=50kJ 2(CH)3OH(.ℓ .)+3O2(.g.) arrow 4H2O(.ℓ .)+2(CO)2(.g.);(ΔH)2=-1500kJ What is the value of ΔH for second reaction if water vapour instead of liquid water is formed as product ? (A) -1450kJ (B) 1500kJ (C) -1300kJ (D) -1700kJ

Tardigrade Admin · Accepted Answer

2(CH)3OH+3O2 arrow 4H2O(.g.)+2(CO)2 ΔH=-1500+4× 50 =-1500+200 =-1300kJ

Q. Consider the following reaction :
$H_{2} O (ℓ) \to H_{2} O (g); (Δ H)_{1} = 50 k J$
$2 (C H)_{3} O H (ℓ) + 3 O_{2} (g) \to 4 H_{2} O (ℓ) + 2 (CO)_{2} (g); (Δ H)_{2} = - 1500 k J$
What is the value of $Δ H$ for second reaction if water vapour instead of liquid water is formed as product ?

$- 1450 k J$

$1500 k J$

$- 1300 k J$

$- 1700 k J$

$2 (C H)_{3} O H + 3 O_{2} \to 4 H_{2} O (g) + 2 (CO)_{2}$
$Δ H = - 1500 + 4 \times 50$
$= - 1500 + 200$
$= - 1300 k J$

Q. Consider the following reaction : H2​O(ℓ)→H2​O(g);(ΔH)1​=50kJ 2(CH)3​OH(ℓ)+3O2​(g)→4H2​O(ℓ)+2(CO)2​(g);(ΔH)2​=−1500kJ What is the value of ΔH for second reaction if water vapour instead of liquid water is formed as product ?

−1450kJ

1500kJ

−1300kJ

−1700kJ

2(CH)3​OH+3O2​→4H2​O(g)+2(CO)2​ ΔH=−1500+4×50 =−1500+200 =−1300kJ

$- 1450 k J$

$1500 k J$

$- 1300 k J$

$- 1700 k J$

$2 (C H)_{3} O H + 3 O_{2} \to 4 H_{2} O (g) + 2 (CO)_{2}$
$Δ H = - 1500 + 4 \times 50$
$= - 1500 + 200$
$= - 1300 k J$