Question

if
15.00 g of MgSO4*7H2O (s) are heated until all waters are released
to the air, how many moles of water were lost from the original
compound

Answer #1

Epsom salt has the formula of MgSO4·7H2O. A 5.45 g sample was
heated and dried completely. After cooling the mass was 2.69 g.
Using calculations, show that the experimental results confirm the
formula for the hydrate (i.e., seven moles of water per MgSO4
formula unit). What is the mass percent of water in the original
salt sample?

Epsom salts is a hydrated ionic compound with the following
formula: MgSO4⋅xH2O A sample of Epsom salts with a mass of
4.93 g was heated to drive off the water of hydration. The mass of
the sample after complete dehydration was 2.41 g.
What is the mass of the water lost during heating?
how many moles of water were lost during
heating?
What is the mass of MgSO4
remaining in the crucible after heating?
How many moles of MgSO4
are...

upon heating 125 g MgSO4 ×7H2O how many grams of water
can be obtained

A 2.540 g sample of an oxide of tin was heated in the air until
the mass of the sample no longer changed, and 2.842 g of tin (IV)
oxide (SnO2) was obtained as a result of the
heating.
Work through the following questions. You only will be asked to
submit your answers to some of them, but you may need to calculate
all of the answers a) - f) to determine the final answer g).
a) What is the...

1. A 5.25g sample of magnesium sulfate hydrate is heated until
the masses stabilize. If the residue has a mass of 2.56g, answer
the following. Show your formula and then how your data is
substituted into the formula.
? What is the mass of the original hydrate?
? What is the mass of the anhydrous salt?
? What mass of water was removed?
? What percentage of the compound was water?
? How many moles of water were removed?
?...

A 2.815-g sample of CaSO4 . XH20 was heated until all of the
water was removed. Calculate the percentage water of hydration and
the formula of the hydrate if the residue after heating weighed
2.485g.

4.430g mixture containing CaCO3 (s) is heated until
all CaCO3 (s) is decomposed completly.
CaCO3 (s) >>>> CaO (s) +
CO2 (g) (Molar mass: CaCO3= 100.0g/mol CaO=
56.1g/mol CO2= 44.0g/mol)
If the mass of the mixture remaining after heating is 3.580g,
calculate the percent CaCO3 in the mixture from
the mass loss of the sample.

Carbon disulfide and carbon monoxide are produced when carbon is
heated with sulfur dioxide. 5C(s)+2SO2(g)→CS2(l)+4CO(g).
a. How many moles of C are needed to react with 0.460 mole
SO2
b. How many moles of CO are produced when 1.4 moles C
reacts?
c. How many moles of SO2 are required to produce 0.50 mole
CS2?
d.How many moles of CS2 are produced when 2.6 moles C
reacts?

Empirical Formula of Epsom Salt
Introduction
Hydrates are crystalline solids that contain a fixed number of
water molecules as an integral part of their crystalline structure.
The number of water molecules bound per metal ion is often
characteristic of that particular metal ion. One of the common
hydrates is hydrated magnesium sulfate (Epsom salt). Epsom salt is
used to reduce inflammation when applied externally.
Epsom salts formula is sometimes written as
MgSO4.xH2O. In this experiment, you
will be trying to...

When solid CaCO3 is heated, it decomposes to give solid
CaO and CO2 gas. A volume of 560 mL of gas is collected over water
at a total pressure of 730 mmHg and 16 ∘C. The vapor pressure of
water at 16 ∘C is 14 mmHg. CaCO3(s)→CaO(s)+CO2(g)
1)How many moles of CO2 gas were in the CO2 gas sample? Express
your answer with the appropriate units

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