For each of the following unbalanced reactions, sup- pose exactly 5.00 g of each reactant is taken. Deter- mine which reactant i
1 answer:
Answer:
The reactant that is limiting is the Na2B4O7, and the mass of the excess reagent (H2SO4) is 2.5627g.
Explanation:
The unbalanced reaction is:
Na2B4O7 + H2SO4 + H2O ⇒ H3BO3 + Na2SO4
- First the equation is balanced
Na2B4O7 + H2SO4 + 5H2O ⇒ 4H3BO3 + Na2SO4
According to the balanced equation we observe that it takes 1 mol of Na2B4O7 to react with 1 mol of H2SO4.
- Then the molecular weights of each reactant are determined:
MWNa2B4O7 = 201.197 g/mol
MWH2SO4 = 98.075 g/mol
- It is calculated how many moles will react with 5 initial grams of each.
201.197 g of Na2B4O7 ⇒ 1 mol
5 g ⇒ X
of Na2B4O7
98.075 g of H2SO4 ⇒ 1 mol
5 g ⇒ X
of H2SO4
The limiting reagent is the one that is consumed first, in this case it is Na2B4O7, since 0.02485 moles are needed for both reactants, then there are 0.02613 moles of H2SO4 left over. With these moles the grams of excess reagent are calculated.
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Answer:
Sample C is most likely the metal.
Explanation:
The Sample C is the metal, because the properties given in the sample c are all of the metal. As we know that the metals are the lustrous or the shiny elements. They are often good conductor of heat and also electricity. The metals possess high melting point. The density of the metals are heavy for their size. Metals can be easily hammered, and hence are malleable. They can easily be stretched into wires hence are ductile. They remains solid at room temperature but in case of mercury it remains as liquid. Metals are opaque object and cannot be see through it.
