Given the chemical reaction
Al + 3AgNO3 → Al(NO3)3 + Ag
how many milliliters of 0.544 M AgNO3 will react with 1.00 g of Al?
Answer in (mL)
Given the chemical reaction Al + 3AgNO3 → Al(NO3)3 + Ag how many milliliters of 0.544...
A. How many moles of Al can be produced from 10.87 g of Ag? Al(NO3)3(aq) + 3 Ag(s) → Al(s) + 3 AgNO3(aq) B. What mass of O2 can be generated by the decomposition of 100.0 g of NaClO3? 2NaClO3(s) → 2 NaCl(s) + 3 O2(g) C. What mass of Fe is generated when 100.0 g of Al are reacted? Fe2O3(s) + 2 Al(s) → 2 Fe(s) + Al2O3(s)
o. Study this chemical reaction: ups ni sorlg dst noitos ollat 3AGNO3(aq) + Al(s) 3Ag(s) +Al(NO3)3(aq) 09:6h) Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. 31 Oxidation: A Al 3e Aate Reduction: Ag
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In a precipitation reaction between Al(NO3)3(aq) and Na2S(aq), 12.7 mL of 0.150 M Al(NO3)3(aq) completly reacted with 10.5 mL of Na2S(aq). What was the molarity of Na2S(aq)? 2 Al(NO3)3(aq) + 3 Na2S(aq) → Al2S3(s) + 6 NaNO3(aq) Note: Insert only the numerical value of your answer with three decimal places (do not include the units or chemical in your answer).
How many milliliters of H2 gas at STP are produced when 0.150 g of Al reacts by the following reaction? 2 Al + 2 OH-1 + 2 H2O = 3H2 + 2 AlOz' (BALANCED) 124 ml 187 ml 62.0 mL 209 ml 141 ml
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