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dlinn [17]
3 years ago
6

How many grams of hcl are produced when 10.0 g of cl2 and 1.00 g of h2 react? h2(g) cl2(g) ---> 2 hcl(g)?

Chemistry
1 answer:
zmey [24]3 years ago
8 0
I belive all you have to do is add cl making 20g then u must also add2.00 because the reactant is 2HCl because the 2 is out front that makes both elements take them equaling 22.00
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Vlad [161]

Answer: bro pic is not cleyer

7 0
3 years ago
An unknown compound contains only C , H , and O . Combustion of 4.20 g of this compound produced 10.3 g CO 2 and 4.20 g H 2 O .
vodomira [7]

Answer:

C4H8O

Explanation:

We can get the answer through calculations as follows.

From the mass of carbon iv oxide produced, we can get the number of moles of carbon produced. We first divide the mass by the molar mass of carbon iv oxide. The molar mass of carbon iv oxide is 44g/mol

The number of moles of carbon iv oxide is 10.3/44 = 0.2341

Since there is only one carbon atom in CO2, the number of moles of carbon is same as above

The mass of carbon in the compound is simply the number of moles multiplied by the atomic mass unit. The atomic mass unit of carbon is 12. The mass of carbon in the compound is thus 12 * 0.2341= 2.8091

From the number of moles of water, we can get the number of moles of hydrogen. To get the number of moles of water, we need to divide the mass of water by its molar mass. Its molar mass is 18g/mol. The number of moles here is thus 4.2/18 = 0.2333

But there are 2 atoms of hydrogen in 1 mole of water and thus, the number of moles of hydrogen is 2 * 0.2333 = 0.4667 moles

The mass of hydrogen is thus 0.4667* 1 = 0.4667

The mass of oxygen equals the mass of the compound minus that of hydrogen and that of carbon.

= 4.2 - 0.4667 - 2.8091 = 0.9242

The number of moles of oxygen is the mass of oxygen divided by its atomic mass unit.

That equals 0.9242/16 = 0.0577625 moles

The empirical formula can be obtained by dividing the number of moles of each by the smallest which is that of oxygen

H = 0.4667/0.0577625 = 8

O = 0.0577625/0.0577625 = 1

C = 0.2341/0.0577625 = 4

The empirical formula is thus C4H8O

5 0
3 years ago
A) Of options (a) - (d) below, highlight the (unbalanced) chemical equation that represents
labwork [276]

Answer:

c...............

Explanation:.............................yuuuuuuuuuuuuuuuuuuuuuwoopuuuuuuuu

7 0
3 years ago
Which hand is negatively changed?<br><br> A.<br> B.<br> C.<br> D.
Lemur [1.5K]

Answer:

I think B

Explanation:

There are more negative ions than positive ions

6 0
3 years ago
How many moles of ideal iodine gas has a volume of 1250 mL at 10 degrees C and 768 mm pressure?
SSSSS [86.1K]

Answer:

n=0.0564mol

Explanation:

Hello,

In this case, since iodine is ideal we can use the ideal gas equation to compute the moles at the given conditions, considering the following units:

V=1250mL*\frac{1L}{1000mL} =1.25L\\P=768mmHg*\frac{1atm}{760mmHg}=1.01atm\\ T=10+273.15=283.15K

PV=nRT

n=\frac{PV}{RT} =\frac{1.01atm*1.25L}{0.082\frac{atm*L}{mol*K}*273.15K}  \\\\n=0.0564mol

Best regards.

5 0
3 years ago
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