Which of the following is a balanced chemical reaction? A 1H_(2)O_(2)grave (a)1H_(2)O+1O_(2) B 2H_(2)O_(2)grave (a)2H_(2)O+O_(2) C 2H_(2)O_(2)grave (a)1H_(2)O+2O_(2) D 4H_(2)O_(2)grave (a)4H_(2)O+2O_(2)
Solution4.7(234 votes)
Answer
Explanation
Similar Questions
Different compounds having the same molecular formula are called __ isomers isomeric compounds isomonomers isosceles
1. What is electronegativity? a. An atom's distance from the nucleus to its valence electron cloud b. The amount of energy needed to remove a valence electron c. The trend of how many electrons are in the outermost ring d. The ability to be able to gain electrons to reach stability
When 24 g of methane gas $(CH_{4})$ is combined with 16 g of oxygen gas, if 15 g of water is collected and the only other product is carbon dioxide, how much carbon dioxide must have been released? 25 a 2.09 40 g 15g
A(n) __ is matter composed of two or more substances that can be separated by physical means. element substance mixture compound
Mercerization of cotton fibers: All statements are correct chemical treatment will cause the fibers to swell will change the shape of cotton fibers fibers become more lustrous and absorbent
Lithium and nitrogen react in a combination reaction to produce lithium nitride: $6Li(s)+N_{2}(g)\rightarrow 2Li_{3}N(s)$ How many moles of lithium are needed to produce 21.0 mol of $Li_{3}N$ when the reaction is carried out in the presence of excess nitrogen? 42.0 mol 63.0 mol 7.00 mol 14.0 mol 21.0 mol
How many neutrons are in Uranium isotopes? 146 Mass minus 92 Same \#neutrons in every isotope
5. According to nutritional guidelines from the US Department of Agriculture, the estimated average requirement for dietary potassium is 4.7 g. What is the estimated average requirement of potassium in moles?
If a reaction is first order with a rate constant of $0.0450$ $s^{-1}$ how much time is required for $75\% $ of the initial quantity of reactant to be consumed? Answer: $\square $ S
Calculate the percent yield of $Br_{2}$ for the chemical reaction $2AgBr\rightarrow 2Ag+Br_{2}$ if the actual yield is 2.147 g and you start Ewith 6.234 g of AgBr.