How many grams of #N_2# are produced from the reaction of 8.96 g of #H_2O_2# and 6.68 g of #N_2H_4#?
Approx.
Hydrazine is OXIDIZED to dinitrogen gas...
Hydrogen peroxide is REDUCED to water...
And so now we assess the molar quantities of each reagent...
And thus hydrogen peroxide is the reagent in MOLAR deficiency (why they could not have added excess is beyond me!)….
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To find the amount of N2 produced, first, calculate the moles of H2O2 and N2H4 using their molar masses. Then, determine the limiting reactant. Once you have the limiting reactant, use the stoichiometry of the balanced chemical equation to find the moles of N2 produced. Finally, convert moles of N2 to grams using its molar mass.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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