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How to do this question?

when 110g of Mn dissolving in dil HNO3 at 27 C under atmospheric pressure, the work done is?

a)2494.2J

b)-2494.2J

c)-4988.4J

d)4988.4J

The heats of formation of F2O (g), H2O(g) and HF (g) are 5.5 kcal, –57.8kcal and 64.2 kcal respectively.

(A) 76.1 Kcal

(B) 11.9 Kcal

(C) 71.6 Kcal

(D) 91.1 Kcal

${H}_{2}\left(g\right)+C{l}_{2}\left(g\right)\to 2HCl\left(g\right)\u2206H\xb0=-185kJ$

If 3 moles of H

_{2}completely react with mole of Cl_{2}to form HCl. What is $\u2206U\xb0$ the for this reaction ?(A) 0 (B) -185 kJ (C) 555 kJ (D) None of these

1.delta H

2. work done on water vapour

3. heat of vapourization

4. delta U

ΔH° sublimation of Mg(s) is 148 (kJ/mol)

ionization energy of is Mg 2187 (kJ/mol)

vaporization of Br2(l) is 31 (kJ/mol)

dissociation of Br2(g) is 193 (kJ/mol)

electron gain enthalpy of Br(g) is 331 (kJ/mol)

ΔH° for MgBr2(s) is 524(kJ/mol)

18.What is the work done $\left(\left|w\right|\right)$ of 1 mole of monoatomic ideal gas in a process described by given V-T graph.Use R = 2 cal/mol K, ln 2 = 0.7

(A) 500 cal

(B) 760 cal

(C) 660 cal

(D) 600 cal

Fe2O3(s) + 3H2 (g) ---- 2Fe(s) + 3H2O(g)

delta H =98.8 Kj and delta S =141.5 J/K

which is correct for above reaction

(1) spontaneous above 298 K (2) spontaneous below 298 K

(3) spontaneous below 698 K (4) spontaneous above 698 K

(A) -76.5 Kcal

(B) -11.9 Kcal

(C) -71.6 Kcal

(D) -91.1 Kcal

are graphical questions neceessary for iit???

_{2 }in a vessel at 300k. how much heat (in terms of R) is required to increase the rms speeds of these molecules to become the double their initial values? also calculate the final temperaturesOne mole of napthalene was burnt in oxygen gas at

to give CO2 gas and water at 25 C. The heat evolved was found to be 5138.8kJ.Calculate the heat of reaction atconstant volumeconstant pressure.Q. 3 Find the heat of formation of ethyl alcohol from following data :

$C\left(s\right)+{O}_{2}\left(g\right)\to C{O}_{2}\left(g\right).\u25b3H=-94kcal\phantom{\rule{0ex}{0ex}}{H}_{2}\left(g\right)+\frac{1}{2}{O}_{2}\left(g\right)\to {H}_{2}O\left(\mathcal{l}\right).\u25b3H=-68kcal\phantom{\rule{0ex}{0ex}}{C}_{2}{H}_{5}OH\left(\mathcal{l}\right)+3{O}_{2}\left(g\right)\to 2C{O}_{2}\left(g\right)+3{H}_{2}O\left(\mathcal{l}\right).\u25b3H=-327kcal$

chemistry part 1 class 11pg no.183

q no 6.14

please can u solve this i am not getting how to do it

consider the oxidation of iron metal at 25 degree celsius 4Fe (s) + 2O2 (g) ---- 2Fe2O3(s) and delta H =-1648.4 Kj

from the given data , under given conditions . delta S of Fe , O2, and Fe2O3 are 27.3 ,205, and 87.4 J/Kmolreaspectively, above reaction is

(1) spontaneous (2) non-spontaneous

(3) at equllibrium (4) cannot be predicted

7. The difference between heat of reaction at constant volume and constant pressure of the reaction.

${\mathrm{C}}_{2}{\mathrm{H}}_{2}\left(\mathrm{g}\right)+\frac{5}{2}{\mathrm{O}}_{2}\left(\mathrm{g}\right)\to 2{\mathrm{CO}}_{2}\left(\mathrm{g}\right)+{\mathrm{H}}_{2}\mathrm{O}\left(\mathrm{l}\right)$

At 300 K in Kcal is [Given: R=2 cal/mol. K]

(A) -0.3 Kcal (B) +0.3 Kcal (C) -0.9 Kcal (D) None of these.