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Vesna [10]
3 years ago
7

Which is the correct molar mass for the compound h2SO4

Chemistry
1 answer:
AlladinOne [14]3 years ago
4 0

Explanation: just add the atomic masses on the periodic table together for each atom.

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6.The original Listerine formula contains 26.9% alcohol (v/v). How many liters of Listerine can be prepared from 4.5 L of pure a
Burka [1]

Answer:

Amount of Listerine can be prepared = 16.73 (Approx)

Explanation:

Given:

Listerine formula contains = 26.9% alcohol

Amount of alcohol = 4.5 L

Find:

Amount of Listerine can be prepared

Computation:

Amount of Listerine can be prepared = (Amount of alcohol) / (Listerine formula contains)

Amount of Listerine can be prepared = 4.5 / 26.9%

Amount of Listerine can be prepared = 16.73 (Approx)

5 0
3 years ago
A real gas behaves least like an ideal gas under the conditions of
Montano1993 [528]

Answer: Option (2) is the correct answer.

Explanation:

A real gas behaves least like an ideal gas under the conditions of low temperature and high pressure.

This is because at low temperature and high pressure molecules of gas will have negligible kinetic energy and strong force of attraction. Thus, real gas will not behave like an ideal gas.

Whereas at high temperature and low pressure a real gas will behave like an ideal gas.


7 0
4 years ago
Read 2 more answers
A 1.25-g sample contains some of the very reactive compound Al(C6H5)3. On treating the compound with aqueous HCl, 0.951 g of C6H
Oksanka [162]
<span>83.9% First, determine the molar masses of Al(C6H5)3 and C6H6. Start by looking up the atomic weights of the involved elements. Atomic weight aluminum = 26.981539 Atomic weight carbon = 12.0107 Atomic weight hydrogen = 1.00794 Molar mass Al(C6H5)3 = 26.981539 + 18 * 12.0107 + 15 * 1.00794 = 258.293239 g/mol Molar mass C6H6 = 6 * 12.0107 + 6 * 1.00794 = 78.11184 g/mol Now determine how many moles of C6H6 was produced Moles C6H6 = 0.951 g / 78.11184 g/mol = 0.012174851 mol Looking at the balanced equation, it indicates that 1 mole of Al(C6H5)3 is required for every 3 moles of C6H6 produced. So given the number of moles of C6H6 you have, determine the number of moles of Al(C6H5)3 that was required. 0.012174851 mol / 3 = 0.004058284 mol Then multiply by the molar mass to get the number of grams that was originally present. 0.004058284 mol * 258.293239 g/mol = 1.048227218 g Finally, the weight percent is simply the mass of the reactant divided by the total mass of the sample. So 1.048227218 g / 1.25 g = 0.838581775 = 83.8581775% And of course, round to 3 significant digits, giving 83.9%</span>
8 0
3 years ago
What salt would form when each of the following
eduard
A.KCl
b.RbNO3
c.NaCl
d.CsBr
4 0
3 years ago
PLEASE HELP!!!!!!!!!!! WILL AWARD 50 POINTS!!!!!!!!!111
Vinil7 [7]

I am pretty sure the answer is . But I might be wrong.

3 0
3 years ago
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