What is the molar mass of C4H10? Enter your answer using
dimensions of molar mass.
For the reaction shown, calculate how many moles of NO2 form
when each amount of reactant completely reacts.
2N2O5(g)→4NO2(g)+O2(g)
4.99×103molN2O5 Express your answer using three significant
figures.
1.011×10−3molN2O5 Express your answer using four significant
figures.
What is the molar mass of the acid if a titration of 4.12 g of
an acid requires 49.29mL of 0.250M NaOH to reach the equivalence
point?
At a certain temperature the Ksp of
Ni(OH)2 is 6.35 x 10-16. What is the molar
soliubility of nickel(II) hydroxide in water in units of M
(mol/liter)?
At a ceratin temperature the solubility of
Ag3PO4 is 4.08 x 10-5M. What is
the Ksp at this temperature?
What mass of a weak acid with a molar mass of 100 g/mol is
necessary to neutralize 25 ml of 0.10 M NaOH solution?
What is the pH of 0.15 g of sodium acetate NaC2H3O2 in 100 ml
water H2O?
Molar Mass by Freezing Point Depression I am doing a latenite
lab on Molar Mass by Freezing Point Depression. I have asked this
question on Course Hero and twice on Chegg and the tutors keep
giving me different answers. Sample 2 has a van't Hoff factor of 2.
It began freezing at -3.6. I added 2 g of the unknown to 10 mL of
water. I was given that the Kf for water is 1.86.
Calculate the molar mass of...
Find the following information for the compound Na2S:
a. What is the molar mass of the compound?
b. How many moles of Na+ ions are there in 223g of the
compound?
c. How many S2- ions/atoms are there in part b?
d. If the compound is reacted with Lead(II) nitrate, what are
the complete and net
ionic equations?
What would be the effect of each of the following on the
calculated molar mass of the solute?
1. some cyclohexane evaporated while the freezing point of pure
cyclohexane was being measured.
2. some cyclohexane evaporated after the solute was added.
3. some unknown power was still left one the weighing paper.
4. a foreign solute was already present in the cyclohexane?
5. the thermometer is not calibrated correctly. it gives a
temperature that is 1.5 C too low at...
Ethanol, C2H5OH (molar mass = 46 g/mol) is mixed with methanol,
CH3OH (molar mass = 32 g/mol) to make an ideal solution at a given
temperature. If 5.00 g of ethanol and methanol are mixed, what is
the resulting vapor pressure of the solution? (the vapor pressure
at the same temperature for pure ethanol is 44.5 mm Hg and pure
methanol is 88.7 mm Hg)
What is the effect on your calculated molar mass if
the following happened:
a. The team lost some t-butanol solvent prior to
adding the solid unknown and starting the determination of the
freezing point of the solute/solvent mix but kept the original
t-butanol mass in their calculations.
b. The team massed out 0.9000g of unknown solute but
only got 0.7000g into the t-butanol solvent but used the 0.9000g in
their calculations.
1.
a. The compound X3Y is 35.0% X. What is the molar
mass of Y if the molar mass of X is 62.4 g/mol?
b. What is the atomic mass of element X if 9.94 g
XCl3 contains 3.26 g X?
c. A 2.953-g sample of an oxide of V contains 1.654 g V. What is
the empirical formula of the oxide?
d. What is the empirical formula of a hydrocarbon if complete
combustion or 6.900 mg of the hydrocarbon...