Iodine reacts with chlorine to form iodine monochloride according to the following unbalanced reaction:
I2 (s) + Cl2 (g) → ICl(g)
If we start with 25.4 g of iodine and 37.4 g of chlorine, how many grams of the excess reactant are leftover after the reaction is complete?
Answer in 3 significant figures:
Iodine reacts with chlorine to form iodine monochloride according to the following unbalanced reaction: I2 (s)...
chemistry limiting reactant question 3 Nitrogen monoxide reacts with chlorine to form nitrosyl chloride according to the following Unbalanced reaction, Nog)+ Cl2(g) → Nocle) 1 If we start with 12.56 of nitrogen monoxide and 17,8 g of chlorine. how many grams of the excess reactant are leftover after the reaction is complete?
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2=0.25 atm and PCl2=0.25 atm . You may want to reference (Page) Section 15.8 while completing this problem. Part A What is the partial pressure of iodine monochloride when the reaction reaches equilibrium? Express your answer to two significant figures and include the appropriate units. atm SubmitPrevious AnswersR
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