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b. NaOH+HClarrow NaCl+H_(2)O 7. If there are 30 grams of iron, 40 grams of water, and 50 grams of iron oxide, how many grams of hydrogen gas are produced? Fe+H_(2)Oarrow Fe_(2)O_(3)+H_(2) a. 20 C. 40 b. 30 d. 50 sides of the equation.

Problemas

b. NaOH+HClarrow NaCl+H_(2)O
7. If there are 30 grams of iron, 40 grams of water, and 50 grams of iron oxide, how many grams of
hydrogen gas are produced?
Fe+H_(2)Oarrow Fe_(2)O_(3)+H_(2)
a. 20
C. 40
b. 30
d. 50
sides of the equation.

b. NaOH+HClarrow NaCl+H_(2)O 7. If there are 30 grams of iron, 40 grams of water, and 50 grams of iron oxide, how many grams of hydrogen gas are produced? Fe+H_(2)Oarrow Fe_(2)O_(3)+H_(2) a. 20 C. 40 b. 30 d. 50 sides of the equation.

Solución

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Elisabethavanzado · Tutor durante 1 años
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To solve this problem, we need to use the law of conservation of mass, which states that the total mass of the reactants must be equal to the total mass of the products.<br /><br />Given information:<br />- 30 grams of iron (Fe)<br />- 40 grams of water (H2O)<br />- 50 grams of iron oxide (Fe2O3)<br /><br />The balanced chemical equation for the reaction is:<br />$Fe + H_{2}O \rightarrow Fe_{2}O_{3} + H_{2}$<br /><br />To find the mass of hydrogen gas (H2) produced, we can use the following steps:<br /><br />1. Calculate the total mass of the reactants:<br /> Total mass of reactants = Mass of Fe + Mass of H2O<br /> Total mass of reactants = 30 g + 40 g = 70 g<br /><br />2. Calculate the total mass of the products:<br /> Total mass of products = Mass of Fe2O3 + Mass of H2<br /> Total mass of products = 50 g + Mass of H2<br /><br />3. Apply the law of conservation of mass:<br /> Total mass of reactants = Total mass of products<br /> 70 g = 50 g + Mass of H2<br /> Mass of H2 = 70 g - 50 g = 20 g<br /><br />Therefore, the mass of hydrogen gas (H2) produced is 20 grams.<br /><br />The correct answer is:<br />a. 20
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