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irina [24]
3 years ago
7

Why is the atomic mass of most elements not a whole number?

Chemistry
1 answer:
Crank3 years ago
3 0
The atomic mass is the average of the isotopes of the element meaning most averages of isotopes will not be whole numbers
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La formula quimica de la molecula de agua H20 , si H = 1 gramos y O = 16 gramos . Cual es su composicion porcentual ? 88,88 % de
vesna_86 [32]

Answer:

88,88 % de O y 11,11 % de H

Explanation:

La composición porcentual se define como la masa que hay de cada mol de átomo en 100g. Las moles de agua en 100g son:

<em>Masa molar agua:</em>

2H = 2*1g/mol = 2g/mol

1O = 1*16g/mol = 16g/mol

Masa molar = 2 + 16 = 18g/mol

100g H2O * (1mol / 18g) = 5.556 moles H2O.

Moles de hidrógeno:

5.556 moles H2O * (2mol H / 1mol H2O) = 11.11 moles H

Moles Oxígeno = Moles H2O = 5.556 moles

La masa de hidrógeno es:

11.11mol * (1g/mol) 11.11g H

La masa de oxígeno es:

5.556 mol * (16g / 1mol) = 88.89g O

Así, el porcentaje de O es 88.89% y el de H es 11.11%. La opción correcta es:

<h3>88,88 % de O y 11,11 % de H</h3>
7 0
2 years ago
Which change favors the products in this reversible reaction n2o4(g)+58 kj 2no2 (g)?
Ksenya-84 [330]

<span>According to Le Chatelier's Principle, the position of equilibrium moves to counteract the change, the position of equilibrium will move so that the concentration of products of chemical reaction increase, if:</span>

<span>1) increase temperature, because this endothermic reaction.</span>

<span>2) increase concentration of reactant.</span>

<span>3) decrease pressure of the system, so reaction moves to direction where is more molecules.</span>

<span>
</span>

7 0
3 years ago
Read 2 more answers
All of the following are balanced equations. State the
Advocard [28]

Answer: a: reactants Na-2 Cl-2

Products: Na-2 Cl-2;

b: reactants P-1 Cl-13 H-6 Products P-1 H-6 Cl-13

c: reactants P-4 H-12 O-16

Products H-12 P-4 O-16

Explanation: since these equations are balanced the atoms on of element on the reactants side will be same as the atoms of the same element of the product side

7 0
3 years ago
Reacting 35.4 ml of 0.220 m agno3 with 52.0 ml of 0.420 m k2cro4 results in what mass of solid formed
laila [671]
Answer is: 1.29 grams <span>of solid formed.
</span>Chemical reaction: 2AgNO₃(aq) + K₂CrO₄(aq) → Ag₂CrO₄(s) + 2KNO₃(aq).
n(AgNO₃) = c(AgNO₃) · V(AgNO₃).
n(AgNO₃) = 0.220 M · 0.0351 L.
n(AgNO₃) = 0.0078 mol; limiting reactant.
n(K₂CrO₄) = 0.420 M · 0.052 L.
n(K₂CrO₄) = 0.022 mol.
From chemical reaction: n(AgNO₃) : n(Ag₂CrO₄) = 2 : 1.
n(Ag₂CrO₄) = 0.0078 mol ÷ 2.
n(Ag₂CrO₄) = 0.0039 mol.
m(Ag₂CrO₄) = 0.0039 mol · 331.73 g/mol.
m(Ag₂CrO₄) = 1.29 g.

7 0
2 years ago
Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the sys
zaharov [31]

Answer:

No effect will be observed.

Explanation:

Let's consider the following reaction at equilibrium.

CuS(s) + O₂(g) ↔ Cu(s) + SO₂(g)

To assess the effect of increasing the pressure, we need to consider Le Chatelier's Principle: if a system at equilibrium suffers a perturbation, it will shift its equilibrium to counteract the effect of such perturbation.

According to the ideal gas equation, the pressure of a gas is proportional to the number of moles. If we increase the temperature, the system will try to reduce it by shifting the equilibrium towards the side with less gaseous moles. However, in this reaction, we have the same number on gaseous moles on the left side and on the right side (1 mole). As a consequence, the increase in the temperature will have no effect on the equilibrium.

8 0
3 years ago
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