The mass of 3.3 mol of an element is 507.5 g. What of the following is the element?
A) I2
B) F2
C) H2
D) N2
E) O2
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The mass of 3.3 mol of an element is 507.5 g. What of the following is...
For each of the following pairs of molecules, identify, which molecule holds the larger entropy value, and briefly (1-3 sentences) explain why. a. 1 mol of H2 O (l) or 1 mol of H2O (g) (both at 100 C) b. 1 mol of I2 (g) or 1 mol of F2 (g) c. 3 mol of O2 (g) or 2 mol of O2 (g) d. 1 cup of coffee at 35 C or 1 cup of coffee at 20 C
Practice with Hess's Law and Standard Heats of Formation 1. (Example) The reaction C2H4 (g) + 6 F2 (g) → 2 CF4(g) + 4 HF (g) can be written as the sum of: C2H4 (9) ► 2 C(s) + 2 H2 (g) AH = -52.3 kJ/mol 2 C(s) + 4 F2 (9) ► 2 CF4(9) AH = -1360 kJ/mol 2 H2(g) + 2 F2 (g) → 4 HF (a) AH = -1074 kJ/mol C2H4(g) + 6 F2(g) → 2 CF4(g)...
Question 3 1 pts Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (=465 nm). F2 and Cl2 o F2 F2, C12, H2, O2 and N2 F2, Cl2 and H2 F2, Cl2, H2 and 02
8. How many gram Na in 5.00g Na2SO4? A. 0.035 g B. 1.31 g C. 1.62 g D. 0.97 g E. 0.81 g 9. A compound containing only carbon and hydrogen has 85.7 wt% C and 14.3 wt%H. Its molar mass is 56 amu. What is its molecular formula? A. C4H8 B. C2H4 C. C2H D. CH2 E. CH 10. Balance the following reactions. No fractional coefficients, coefficients must be the lowest whole numbers. a) ____K + ____H2O →...
Determine ΔrH° for the following reaction, 2 NH3(g) + 5/2 O2(g) → 2 NO(g) + 3 H2O(g) given the thermochemical equations below. N2(g) + O2(g) → 2 NO(g) ΔrH° = +180.8 kJ/mol-rxn N2(g) + 3 H2(g) → 2 NH3(g) ΔrH° = –91.8 kJ/mol-rxn2 2H2(g) + O2(g) → 2 H2O(g) ΔrH° = –483.6 kJ/mol-rxn a. –1178.2 kJ/mol-rxn b. –452.8 kJ/mol-rxn c. –394.6 kJ/mol-rxn d. –211.0 kJ/mol-rxn e. +1178.2 kJ/mol-rxn
Compound X'has a molar mass of 579.43 g mol and the following element | mass % phosphorus 26.73% nitrogen | 12.09% chlorine 61. 1896 Write the molecular formula of X
Using the equation 2H2(g) + O2(g) --> 2H2O(g), what formula would I use to find the mass needed of H2 to react with 13.5 g O2? A. 13.5 g O2 x 1 mol O2 x 1 mol H2 x 2 g H2 1 32 g O2 2 mol O2 1 mol H2 B. 13.5 g O2 x 32 g O2 x 2 mol H2 x 2 g H2 1 1 mol O2 1 mol O2 1 mol H2 C. 13.5 g O2...
What is the molecular mass (in g/mol) of a gaseous element if 4.10 g occupies 7.41 L at 534.80 torr and 39.6 oC?
1.At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3)3COH(g) (CH3)2CCH2(g) + H2O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature? A. The forward reaction will proceed in order to reestablish equilibrium. B. The reverse reaction will proceed in order to reestablish equilibrium. C. No change occurs. D. The equilibrium constant will increase. E. The equilibrium constant will decrease. 2. The following reaction is...
the mass of 1.250 mol of an element is 88.64g. what is the
element
, Ch6, and Ch 7 for Exam 3-20 extra credits lonecia Stevenson: Attempt 1 Previous Page Next Page Page Question 1 (1 point) The mass of 1.250 mol of an element is 88.64 g. What is the element? Ge Osr OBr2 Cl2 O Ga Page Next Page Previous Page Submit Quiz 0 of 30 questions saved DOLL