How many moles of aluminum are required to completely react with 107 mL of 6.00 M H$_2$SO$_4$ according to the balanced chemical reaction: 2 Al(s) + 3 H$_2$SO$_4$(aq) $\rightarrow$ Al$_2$(SO$_4$)$_3$(aq) + 3 H$_2$(g)
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To do this, we need to use the molarity (M) of the H2SO4 solution. The molarity is given as 6.00 M, which means there are 6.00 moles of H2SO4 in 1 liter of solution. We can use the following equation to convert the volume of H2SO4 to moles: moles = volume (in Show more…
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How many moles of aluminum are required to completely react with 107 mL of 6.00 M H2SO4 according to the balanced chemical reaction: 2Al(s) + 3H2SO4(aq) -> Al2(SO4)3(aq) + 3H2(g) STARTING AMOUNT ADD FACTOR ANSWER RESET 428 0.428 1000 0.001 6.00 0.963 107 98.08 0.0374
Ma Ednelyn L.
how many moles of aluminum are required to completely react with 107 mL of 6.00 M H2SO4 according to the balanced chemical reaction: 2 Al (s) + 3 H2SO4 (aq) --> Al2(SO4)3 (aq) + 3 H2 (g)
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