3.7. methanol is synthesized commercially from co and h2 by the reaction co+ 2h2 ch2oh over a cu/zno catalyst at 350°c at 50-100 atm. the standard- state thermodynamic data on this reaction are -90.64 kj/mol and -24.2kj/mol (a) what is the equilibrium conversion of a stoichiometric mixture of co and h2 to methanol at 298 k at 1 atm? (b) assuming ahg independent of t, what are keq and the equilibrium conversion at 1 atm and 350°c? (c) kg at 350°c is measured to be 1.94104. how large is the error assuming constant ahr? (d) at what pressure will the equilibrium conversion be 50% at 350°c?

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

answerto predict;

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally