N2H4 (L) -----> NH3 (g) + N2 (g) How do you balance the equation?  I also need to be able to classify the reaction as either combination, decomposition, single-displacement or double-displacement?

The Apollo 13 mission astronauts are running out of oxygen and need to get rid of the excess carbon dioxide. You know that sodium hydroxide can remove carbon dioxide from the spacecraft cabin. The filter which they had been using is fully saturated and no longer works. The astronauts have a 5 kg container of sodium hydroxide on the ship. The reaction to neutralize the air, remove carbon dioxide with sodium hydroxide is shown below CO2(g) + 2NaOH(s) ⟶⟶ Na2CO3(aq) + H2O(l)   The astronauts have 2 days left before they land on earth. You know that there are three astronauts, and each astronaut emits roughly 500. g of carbon dioxide each day. Is there enough sodium hydroxide in the cabin to cleanse the cabin air of the carbon dioxide, or are the astronauts doomed? Calculate how much sodium hydroxide is required to remove all the carbon dioxide from the three astronauts.  Be sure to show all your work!

CH4​(g)+2 O2​(g) → CO2​(g)+2 H2​O(g)+energy What type of reaction is this?   Single displacement   Combustion   Combination   Double displacement   Decomposition

Which of the following correctly classify the following reaction? (There could be more than one answer) Zn(s) + 2HCl(aq) -->  H2(g) + ZnCl2(aq) Acid/Base reaction Combustion reaction single displacement reaction double displacement reaction gas evolving reactions precipitation reaction

O SIMPLE REACTIONS Identifying precipitation, combustion and acid-base reactions Classify each chemical reaction: type of reaction (check all that apply) reaction O combination O precipitation O single replacement O double replacement O decomposition combustion CH, (g) + 20, (g) → co, (g) + 2H,0(g) O acid-base O combination Oprecipitation O single replacement O double replacement HI(aq) + NaOH (aq) - Nal (aq) + H,0(1) O combustion acid-base decomposition combination O precipitation Fes o, (aq) + PbCl, (aq) → FeCl, (aq) + PbSO,(s) O single replacement O combustion double replacement O acid-base decomposition combination Oprecipitation 4Na(s) + 0, (g) → 2Na,0(s) O single replacement O combustion double replacement Oacid-base decomposition O O Oロ□

Balance the following reaction in basic solution then enter the coefficients of the balanced reaction into the blank spaces. Remember to include "understood" coefficients of 1! 9. Type your answer here Ag20(s) + Type your answer here Al(s) + Type your answer here OH (aq) + H20(1) → Type your answer here Type your answer here Ag(s) + Type your answer here H2A!O3 (aq)

Choose the reaction type(s) for the following reaction.  Be sure to choose all that apply! H2CO3 (aq) ⟶ CO2 (g) + H2O (l) neutralization single replacement precipitation combination decomposition double displacement

Classify each chemical reaction: Ba (CIO,),(s) → BaCl,(s) + 30, (8) KOH(aq) + HBrO (aq) 1 reaction CuSO4 (aq) + Zn CrO4 (aq) K BrO (aq) + H₂O (1) CH₂OCH₂ (1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) ZnSO4 (aq) + Cu Cro(s) type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition 000 000 000 precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base

Classify each of the reactions represented by the following equations, first as a redox or non redox reaction. Then further classify each redox reaction as a decomposition, single-replacement, or combination reaction, and each nonredox reaction as decomposition, double replacement or combination reaction:  CaO(s) + SiO2(s) - > CaSiO3(s)

Balance this reaction.  If a coefficient is one, enter "1" explicitly.   N2+H2 → NH3