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I am Lyosha [343]
2 years ago
6

Which substance could any excess not be removed by filtration​

Chemistry
1 answer:
horrorfan [7]2 years ago
6 0

Answer:

sodium hydroxide

Explanation:

i think sodium hydroxide

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Use the equation to determine what mass of FeS must react to form 326 g of FeCl2.
iogann1982 [59]

Answer:

We need 226 grams of FeS

Explanation:

Step 1: Data given

Mass of FeCl2 = 326 grams

Molar mass FeCl2 = 126.75 g/mol

Step 2: The balanced equation

FeS + 2 HCl → H2S + FeCl2

Step 3: Calculate moles FeCl2

Moles FeCl2 = 326 grams / 126.75 grams

Moles FeCl2 = 2.57 moles

Step 4: Calculate moles FeS needed

For 1 mol H2S and 1 mol FeCl2 produced, we need 1 mol FeS and 2 moles HCl

For 2.57 moles FeCl2 we need 2.57 moles FeS

Step 5: Calculate mass FeS

Mass FeS = 2.57 moles * 87.92 g/mol

Mass FeS = 226 grams FeS

We need 226 grams of FeS

4 0
3 years ago
The scientist most often credited with the idea that a quantum of light (photon) can act as a particle is:
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C.) It was Einstein who created quantum of light
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2 years ago
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A sample of helium gas has a volume of 620. Ml at a temp of 500 K. If we decrease the temperature to 100K while keeping the pres
Ne4ueva [31]

Answer:

A sample of helium gas has a volume of 620mL at a temperature of 500 K. If we ... to 100 K while keeping the pressure constant, what will the new volume be?

Explanation:

3 0
3 years ago
a sample of compound determined to contain 1.71 g C and 0.287 g H. The corresponding empirical formula is
fiasKO [112]

Answer: The empirical formula is CH_2.

Explanation:

Mass of C = 1.71 g

Mass of H = 0.287 g

Step 1 : convert given masses into moles.

Moles of C = \frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{1.71g}{12g/mole}=0.142moles

Moles of H = \frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.287g}{1g/mole}=0.287moles

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C =\frac{0.142}{0.142}=1

For H =\frac{0.287}{0.142}=2

The ratio of C: H = 1: 2

Hence the empirical formula is CH_2.

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3 years ago
Balance the following equations by inserting the proper coefficients.
Montano1993 [528]
1212. 1212. 1323........

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3 years ago
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