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denis23 [38]
3 years ago
15

HELP PLEASE

Chemistry
1 answer:
Phoenix [80]3 years ago
8 0

<u>mass of reactants = mass of products</u> best represents the law of conservation of mass

Explanation:

This is a law of thermodynamic that applies to chemical reactions. The mass of the reactants must equal to that of the products because energy/mass cannot be destroyed or created. This is why ideally, chemical reactions should be balanced to conform to this law.

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Which of the following values are not equal to 1 mole?
Gekata [30.6K]

Answer:

none of them are equal to one mole

3 0
3 years ago
Calculate the mass in grams in nine molecules of CH3COOH? Please show how you got your answer.
WINSTONCH [101]
M CH₃COOH: 12u×2 + 1u×4 + 16u×2 =<u> 60u</u>

m 9CH₃COOH: 60u×9 = <u>540u</u>

<em>(1u ≈ 1,66·10⁻²⁴g)</em>
-----------------------------
1u ------- <span>1,66·10⁻²⁴g
540u ---- X
X = 540</span>×<span>1,66·10⁻²⁴g
<u>X = 896,4</u></span><span><u>·10⁻²⁴g


</u>
</span>
7 0
3 years ago
g Gaseous ethane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 2.71 g of ethane i
Kamila [148]

Answer:

6.05g

Explanation:

The reaction is given as;

Ethane + oxygen --> Carbon dioxide + water

2C2H6 + 7O2 --> 4CO2 + 6H2O

From the reaction above;

2 mol of ethane reacts with 7 mol of oxygen.

To proceed, we have to obtain the limiting reagent,

2,71g of ethane;

Number of moles = Mass / molar mass = 2.71 / 30 = 0.0903 mol

3.8g of oxygen;

Number of moles = Mass / molar mass = 3.8 / 16 = 0.2375 mol

If 0.0903 moles of ethane was used, it would require;

2 = 7

0.0903 = x

x = 0.31605 mol of oxygen needed

This means that oxygen is our limiting reagent.

From the reaction,

7 mol of oxygen yields 4 mol of carbon dioxide

0.2375 yields x?

7 = 4

0.2375 = x

x = 0.1357

Mass = Number of moles * Molar mass = 0.1357 * 44 = 6.05g

8 0
3 years ago
Określ typ tlenku (zasadowy,kwasowy,obojętny,amfoter)<br><br> CuO, FeO,Cr2O3,P4O10,MnO2,CaO,CrO3,SO3
AVprozaik [17]

Answer:

hrhrhr

Explanation:

because h&R blok

6 0
3 years ago
At a given temperature, 4.06 atm of H2 and 3.5 atm of Cl2 are mixed and allowed to come to equilibrium. The equilibrium pressure
Llana [10]

<u>Answer:</u> The value of K_p for the given chemical reaction is 0.1415

<u>Explanation:</u>

Equilibrium constant in terms of partial pressure is defined as the ratio of partial pressures of the products and the reactants each raised to the power their stoichiometric ratios. It is expressed as K_p

For a general chemical reaction:

aA+bB\rightarrow cC+dD

The expression for K_p is written as:

K_p=\frac{p_{C}^cp_{D}^d}{p_{A}^ap_{B}^b}

For the given chemical equation:

H_2(g)+Cl_2(g)\rightleftharpoons 2HCl(g)

The expression for K_p for the following equation is:

K_p=\frac{(p_{HCl})^2}{(p_{H_2)}(p_{Cl_2})}

We are given:

p_{HCl}=1.418atm\\p_{H_2}=4.06atm\\p_{Cl_2}=3.5atm

Putting values in above equation, we get:

K_p=\frac{(1.418)^2}{(4.06)\times (3.5)}\\\\K_p=0.1415

The value of K_p for the given chemical reaction is 0.1415

5 0
3 years ago
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