If excess carbon disulfide reacts with 450 mL of oxygen, 150 mL of carbon dioxide and 300 mL of sulfur dioxide gases would be produced respectively.
<h3>Stoichiometric calculation</h3>
The reaction between liquid carbon disulfide and oxygen is represented by the equations below:
The mole ratio of oxygen to carbon dioxide and sulfur dioxide produced is 3:1:2.
Thus, for 450 mL oxygen, 1/3 x 450 = 150 mL of carbon dioxide will be required.
Also for 450 mL of oxygen, 2/3 x 450 = 300 mL of sulfur dioxide will be required.
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The specific heat of aluminum is 0.902 J/gC. E=m*cp*delta T, or
125*0.902*(95.5-19)= 8630 J
Answer: option <span>D Chemical reaction rates vary with the conditions of the reaction, but nuclear decay rates do not.
Justification:
1) The rate of chemical reactions are affected by: concentration of the reactants, state of the reactants, temperature, and presence of catalizers. So the first part of the statement is true.
2) Nuclear decay rates are constant. The decay depends on the nature of the element but not the conditions. That is why dating fossils with radiactive isotopes is possible. So, the second part of the statement is true.
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Answer:
The Equilibrium constant K is far greater than 1; K>>1
Explanation:
The equilibrium constant, K, for any given reaction at equilibrium, is defined as the ratio of the concentration of the products raised to their stoichiometric coefficients divided by the concentration of reactants raised to their stoichiometric coefficients.
It tells us more about how how bigger or smaller the concentration of products is to that of the reactants when a reaction attains equilibrium. From the given data, as the color of the reactant mixture (Br2 is reddish-brown, and H2 is colourless) fades, more of the colorless product (HBr is colorless) is being formed as the reaction approaches equilibrium. This indicates yhat the concentration of products becomes relatively higher than that of the reactants as the reaction progresses towards equilibrium, the equilibrium constant K, must be greater than 1 therefore.
